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3 cards from this section. Quick, good the night before a test.
Define Gibbs free energy.
Think about what energy can be used for in a chemical reaction.
What does the equilibrium constant Kp represent?
Consider how products and reactants relate post-reaction.
What is Gibbs Free Energy?
Think about what happens in a closed system.
If Kp is less than 1, which side does the equilibrium favor?
Remember what Kp signifies about products and reactants.
Given the reaction: N2(g) + 3H2(g) ⇌ 2NH3(g) has an equilibrium constant Kp = 4.5 at 500 K. If the initial concentrations are [N2] = 0.5 M, [H2] = 1 M, and [NH3] = 0, calculate the equilibrium concentrations of all species.
Remember to account for stoichiometry in your x values.
How would increasing temperature affect a reaction with ΔH > 0 in terms of Gibbs free energy?
Consider how temperature interacts with the term -TS in the Gibbs equation.
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